EP2780346A1

EP2780346A1 - Process for preparing metal difluorochelatoborates and use as battery electrolytes or additives in electrochemical cells

Info

Publication number: EP2780346A1
Application number: EP12784274.8A
Authority: EP
Inventors: Ulrich Wietelmann; Peter Rittmeyer; Ute Emmel
Original assignee: Rockwood Lithium GmbH
Current assignee: Albemarle Germany GmbH
Priority date: 2011-11-14
Filing date: 2012-11-14
Publication date: 2014-09-24
Anticipated expiration: 2032-11-14
Also published as: US9260456B2; JP2014533293A; JP6188706B2; CN104185636B; EP2780346B1; DE102012220793A1; US20140288331A1; CA2856123A1; CA2856123C; WO2013072359A1; CN104185636A

Abstract

The invention relates to a process for preparing metal difluorochelatoborates, in which a metal bis(chelato)borate of the formula M[BL₂] is reacted with boron trifluoride and a metal fluoride (MF) and/or a metal salt of the chelating ligand (M₂L) where M+ is a monovalent cation selected from the group consisting of lithium, sodium, potassium and ammonium NR₄ ⁺, where R = H, alkyl (C1 to C8) and L is a chelating agent having two terminal oxygen atoms and having the general formula (II), where: when m = 1 and Y¹ and Y² together with C¹ form a carbonyl group, n = 0 or 1 and o = 0 or 1 and R¹ and R² are each, independently of one another, H or alkyl having from one to eight carbon atoms (C1-C8) and Y³, Y⁴ are each, independently of one another, OR³ (R³ = C1-C8-alkyl), then n or o ≠ 1: p = 0 or 1 and when n and o = 0, p = 1; or Y¹, Y², Y³, Y⁴ are each, independently of one another, OR³ (R³ = C1-C8-alkyl), m = 1, n = 0 or 1, o = 1 and p = 0; or C² and C³ are members of a 5- or 6-membered aromatic or heteroaromatic ring (with N, O or S as heteroelement) which can optionally be substituted by alkyl, alkoxy, carboxy or nitrile, where R¹, R², Y³ and Y⁴ are absent, m = 0 or in the case of 1, Y¹ and Y² together with C¹ form a carbonyl group and p is 0 or 1, in an organic, aprotic solvent.

Description

Process for the preparation of metal difluorochelato borates and use as battery electrolytes or additives in galvanic cells

The invention relates to a process for the preparation of Metalldifluorochelatoboraten and their use as battery electrolytes or additives in galvanic cells.

Mobile electronic devices require ever more powerful rechargeable batteries for independent power supply. In addition to nickel / cadmium and nickel / metal hydride accumulators, lithium batteries are particularly suitable for these purposes, which have significantly higher energy densities compared to the former systems. In the future, large-format lithium batteries should also be used e.g. for stationary applications (power back-up) and in the automotive sector for traction purposes (hybrid drives or purely electric drive). Especially in the latter applications, safety is given paramount importance.

The current generation of lithium-ion batteries uses as the electrolyte a liquid, gel or polymeric electrolyte with LiPF ₆ as conductive salt. This salt begins already when it exceeds about 70 ° C according to

LiPF ₆ LiF + PF ₅ (1) to form the highly reactive Lewis acid PF ₅ to decompose. The acid attacks the organic components of the electrolytes (eg alkyl carbonates) used in the prior art. This reaction is exothermic and can lead to runaway self - heating, which at least impairs the ability of the electrochemical cell to function or causes it to be completely destroyed by dangerous concomitants. As alternative electrolytes, inter alia, solutions of lithium salts with fluorochelatoborate anion, z. Lithium difluorooxalatoborate (LiDFOB) (US6849752, Z. Chen, J. Liu, K. Amine, Electrochem., Solid State Lett.10 (2007) A45-47) or lithium difluoro (1,2-benzene-diolato (2 -) - O, O'-borate (X. Zhao-Ming, J. Power Sources 196 (201 1) 8710).

The following comments focus on the conductive salt LiDFOB. However, they apply analogously to variations of this structure according to the general formula I.

LiDFOB general formula I

M ⁺ is a monovalent cation selected from the group lithium, sodium, potassium or ammonium NR ⁺ , where R = H, alkyl (C1 to C8, acyclic or cyclic)

L is a chelator with two terminal oxygen atoms with the general formula

where m = 1 and Y ¹ and Y ² together with C ^{1 represent} a carbonyl group, n is 0 or 1 and o = 0 or 1 with R ¹ and R ² independently of one another H or alkyl having one to eight carbon atoms ( C1-C8), and Y ^3, Y ⁴ are each independently oR ³ (R ³ = C1-C8 alkyl), then for n or o is 1: p = 0 or 1 and n and o = 0, p = 1 ; or

Y ¹ , Y ² , Y ³ , Y ^{4 are} each independently OR ³ (R ³ = C 1 -C 8 alkyl), m = 1, n = 0 or 1, o = 1 and p = 0; or C ² and C ³ are members of a 5- or 6-membered aromatic or heteroaromatic ring (with N, O or S as a heteroelement) which may be optionally substituted with alkyl, alkoxy, carboxy or nitrile, wherein R ¹ , R ² , Y ³ and Y ⁴ are omitted, m = 0 or in the case of 1, Y ¹ and Y ² together with C ^{1 represent} a carbonyl group and p is 0 or 1. The conductive salt LiDFOB (M ⁺ = Li and L = C ₂ O ₄ ^{2 "} ) can be prepared in various ways.

In the reaction of lithium tetrafluoroborate (LiBF) with 2 equivalents of lithium hexafluoroisopropanolate in acetonitrile, first lithium fluoride (LiF) is eliminated (EP 1 195834). The relatively weakly bound alkoxy ligands of the intermediate product are exchanged in a second step for the better chelate donor oxalate:

A disadvantage of this method is that LiF remains in the product, the ligand 1, 1, 1, 3, 3, 3-hexafluoroisopropanol expensive and the process consuming because it is two-stage. In a further production process, lithium tetrafluoroborate anhydrous oxalic acid and SiCl are reacted as auxiliary reagent (EP 1308449):

2 LiBF + 2 H ₂ Ox + SiCl ₄ Li [F ₂ BO x] + 4 HCl + SiF ₄ A disadvantage of this synthesis is the formation of the acidic and toxic by-products SiF ₄ and HCl: furthermore, chloride traces remain in the product. Chloride is known to be corrosive to aluminum, so that such chloride-contaminated conductive salt corrodes the cathode current collector used in Li-ion batteries, typically an aluminum foil.

It is also known that LiDFOB forms in the warm storage of equimolar mixtures of LiBF and LiBOB in ethylene carbonate / ethyl methyl carbonate (EC / EMC) in a very slow reaction (B. Lucht, Electrochem., Solid State Lett., 14 (11) A161 -A164 (201 1)). Thus, the mixed salt LiDFOB is obtained at 100 ° C storage within 10 weeks with about 80% yield. The disadvantages of this method are that the conversion is significantly too slow for commercial use and that the raw material LiBF is expensive.

In another method, boron trifluoride, usually in the form of an ether adduct, is reacted with lithium oxalate (S.S. Zhang, Electrochem., Commun., 8 (2006) 1423-28):

Li ₂ C ₂ O ₄ + BF ₃ ^■ Donor Li + LiF (4)

(Donor = Et ₂ O or THF)

A disadvantage of this process is that the target product LiDFOB is formed only with a yield of 50% and LiBF is produced to the same extent. The by-product LiF formed according to Equation (Eq.) (4) reacts immediately with boron trifluoride to give LiBF ₄ , so that in total the following reaction equation applies: Li ₂ C ₂ O ₄ + 2 BF ₃ -> Li [F ₂ BC ₂ O ₄ ] + LiBF ₄ (4a)

Finally, LiDFOB can be prepared from lithium tetrafluoroborate and bis (thmethylsilyl) oxalate in acetonitrile solution (C. Schreiner, M. Amereller, H. Gores, Chem. Eur. J. 13 (2009) 2270-2):

Disadvantages of this process are the high costs and the unavailability of the silyl ester and the formation of the by-product trimethylsilyl fluoride.

The object of the invention has been found to provide a method that forms starting from industrially available, easy to handle raw materials Metalldifluorochelatoborate, in particular LiDFOB in a one-step, simple reaction.

The stated object is achieved by using a metal ib / s (chelato) borate of the formula M [BL ₂ ] with boron trifluoride and a metal fluoride (MF) and / or a metal salt of the chelate ligand (M ₂ L) with M ⁺ , a monovalent Cation selected from the group lithium, sodium, potassium or ammonium NR ₄ ⁺ , wherein R = H, alkyl (C1 to C8, acyclic or cyclic) and

L is a chelating agent having two terminal oxygen atoms with the general formula

Y ¹ , Y ² , Y ³ , Y ^{4 are} each independently OR ³ (R ³ = C 1 -C 8 alkyl), m = 1, n = 0 or 1, o = 1 and p = 0; or

C ² and C ³ are members of a 5- or 6-membered aromatic or heteroaromatic ring (with N, O or S as heteroelement), which may optionally be substituted by alkyl, alkoxy, carboxy or nitrile, where R ¹ , R ² , Y ³ and Y ⁴ are omitted, m = 0 or in the case of 1 Y ¹ and Y ² together with C ^{1 represent} a carbonyl group and p is 0 or 1, is reacted in an organic aprotic solvent.

The reactions can be described by the following general equations:

M ₂ L + M [BL ₂ ] + 2 BF ₃ ^► 3 M [F ₂ BL] (6)

MF + M [BL ₂ ] + BF ₃ ^► 2 M [F ₂ BL] (7) In the case of the preparation of the particularly preferred conducting salt LiDFOB, lithium ö / s (oxalato) borate ("LiBOB") is reacted with lithium fluoride or lithium oxalate and boron trifluoride:

Li ₂ C ₂ O ₄ + LiBOB + 2 BF ₃ 3 Li [F ₂ BC ₂ O ₄ ] (8)

LiF + LiBOB + BF ₃ -> 2 Li [F ₂ BC ₂ O ₄ ] (9)

Analogously, the likewise particularly preferred conducting salt lithium difluoromalonato borate (LiDFMB) is prepared from lithium oil (malonato) borate and BF _{3 as} well as LiF or lithium malonate (Li ₂ C ₃ H ₂ O ₄ ). Further preferred products are: lithium difluorolactatoborate, lithium difluoroglycolate borate, lithium difluorosalicylatoborate, lithium difluoroborate catechinatoborate and the corresponding sodium salts. There are aprotic organic solvents, preferably ethers, esters, nitriles, lactones, carbonates, either used in pure form or in any mixture. In addition, hydrocarbons (aromatics or saturated compounds) can be used in mixtures with the aforementioned functionalized solvents.

Very particular preference is given to using solvents which are suitable for use in lithium batteries. These include: carbonic acid esters (dimethyl carbonate, diethyl carbonate, ethyl methyl carbonate, propylene carbonate, ethylene carbonate), cyclic ethers such as tetrahydropyran or tetrahydrofuran, polyethers such as 1, 2-dimethoxyethane or diethylene glycol dimethyl ether, furthermore nitriles such as acetonitrile, adiponitrile, malononitrile, glutaronitrile and lactones such as γ-butyrolactone.

The reaction is carried out at temperatures between 0 and 250 ° C, preferably 20 and 150 ° C and more preferably between 30 and 130 ° C.

The sparingly soluble starting materials, ie the metal fluorides and / or metal chelate salts, are used in pulverized form, preferably ground. The average particle size is preferably <100 μm and particularly preferably <50 μm.

All starting materials, in particular the metal salts and the solvents are used in anhydrous form, ie the water contents of the raw materials are <1000 ppm, preferably <300 ppm. In a particularly preferred embodiment, a catalyst is used to accelerate the reaction. The catalysts used are Lewis acids or substances which are capable of liberating Lewis acids in the reaction mixture. Preferred catalysts are element compounds of the 2nd to 15th group of the Periodic Table, particularly preferably molecular halides, perfluoroalkyls, perfluoroaryls and oxo compounds of boron, aluminum and phosphorus. Examples are: aluminum alcoholates (Al (OR) 3), boric acid esters (B (OR) 3), phosphorus oxides and phosphorus halides. Very particularly preferred are super-acidic boron compounds such as B (C ₆ F ₅ ) ₃ ("BARF"), C ₆ F ₅ BO ₂ C ₆ F ₄ and boric acid esters of trivalent oxygen-based chelating ligands such as

The catalytic use of LiPF ₆ which is in equilibrium with the strong Lewis acid PF ₅ under the abovementioned reaction conditions is also very particularly preferred (equation 1). The catalysts mentioned are used in amounts of at most 20 mol%, preferably up to 10 mol% and particularly preferably up to 5 mol%, based on the boron trifluoride used.

In the following, the process according to the invention will be described in general terms. In anhydrous solvent, the metal salts are presented. With stirring, boron trifluoride is then either introduced in the gaseous state or condensed or metered in the form of commercially available solvate complexes, for example as BF ₃ × diethyl ether, BF ₃ × THF or BF ₃ × acetonitrile. Particularly preferred is the use of gaseous BF ₃ or a previously prepared with BF ₃ gas solution in the desired solvent (eg, a carbonate such as dimethyl carbonate or propylene carbonate). As a result, the entry of a battery electrolyte in unusual or even disturbing solvent such as diethyl ether is avoided. The BF ₃ - dosing takes place in the temperature range between 0 ° C and 150 ° C, preferably between 10 and 100 ° C. After complete addition of the BF ₃ is stirred until the reaction is complete. The progress of the reaction can conveniently be monitored, for example, by ¹¹ B NMR measurements. The process according to the invention may also deviate slightly from the theoretical stoichiometry (Equations 6 to 9). The stoichiometries are preferably selected which lead to a complete consumption of the raw material BF ₃ which interferes with the battery. For this purpose, the metal salts MF and / or M ₂ L are used in excess. The metal salts mentioned are preferably used with 0.1 to 100% by weight excess, more preferably with 1 to 20% by weight.

After complete reaction, the reaction solution is clarified by filtration (e.g., membrane filtration). As such, it can be used directly as a battery electrolyte or additive if no solvents which disturb the battery performance were used. If interfering solvents should be present, the synthesized Metalldifluorochelatoborat invention is obtained by an evaporation or crystallization process in pure form.

The invention will be explained with reference to the following 7 examples.

Example 1: Preparation of LiDFOB from LiBOB, lithium oxalate and BF ₃ in

Dimethyl carbonate (DMC)

In a 0.5 L jacketed reactor equipped with reflux condenser and dropping funnel, 37.5 g of LiBOB and 19.8 g of Li ₂ C ₂ O were placed in 229 g of anhydrous DMC and heated to an internal temperature of 70 ° C. Then 55.0 g of boron trifluoride etherate were added within one hour. The jacket temperature was adjusted so that the reaction mixture boiled gently the entire time. After dosing, further refluxing was carried out and from time to time samples were taken. The samples were checked for reaction progress by ¹¹ B-NMR:

Time of sample -1, 1 ppm * 0 ppm * 3.1 ppm * 7.6 ppm * would take LiBF BF ₃ LiDFOB LiBOB Dosing 41, 5 4,7 42,9 10,8

2 h postreaction 43.0 3.0 45.9 8.2

7.5 h post-reaction 37.8 3.9 47.6 10.7

9 h post-reaction 36.9 2.9 48.4 1 1, 8

1 1, 5 h postreaction 37.7 2.6 55.3 4.5

18.5 h post-reaction 17.6 2.2 66.7 13.6

26 h post-reaction 9.2 1, 9 78.9 8.9

30 h post-reaction 8,8 2,1 81, 4 7,7

* indicates the chemical shift of the respective product in ¹¹ B-NMR

spectrum

After a 30-hour reaction time> 80% d. Th. Formed on LiDFOB and the composition did not change significantly with further stirring. It has thus formed a thermodynamically induced equilibrium mixture. The reaction mixture was filtered and used in this form (clear solution) as the electrolyte for lithium batteries. Example 2: Preparation of LiDFOB from LiBOB, lithium oxalate and BF ₃ in

Dimethyl carbonate (DMC), 5 mol% catalyst LiPF ₆

In an inertized GC-septum glass with magnetic stirrer core, 1.50 g LiBOB and 0.91 g lithium oxalate were dissolved or suspended in 9.16 g DMC and 0.59 g of a 10% LiPF ₆ solution in DMC was added. To the stirred suspension was added 2.20 g of boron trifluoride etherate and then heated to 70 ° C. Samples were taken at certain time intervals and tested for reaction progress by ¹¹ B-NMR: Time of Samples-1, 1 ppm ^* 0 ppm ^* 3.1 ppm ^* 7.6 ppm ^* take LiBF BF ₃ LiDFOB LiBOB

1 h 70 ° C 41, 5 0.5 46 8

5 h 70 ° C 16 1, 1 72 1 1

12 h 70 ° C 14 1, 0 79

^* indicates the chemical shift of the respective product in the B-NMR spectrum Example 3: Preparation of LiDFOB from LiBOB, lithium oxalate and BF ₃ in

Propylene carbonate (PC), with and without 5 mol% catalyst LiPFö

In two inerted GC-septum glasses with magnetic stirrer, in each case 1.50 g of LiBOB and 0.79 g of lithium oxalate were dissolved or suspended in 9.2 g of PC. In one of the vials 0.59 g of a 10% solution of LiPFö in PC were injected. 2.20 g of boron trifluoride etherate were added to the stirred suspensions and then heated to 70.degree. Samples were taken at certain time intervals and tested for reaction progress by ¹¹ B-NMR:

Example 4: Preparation of LiDFOB from LiBOB, lithium fluoride and BF ₃ in

Propylene carbonate (PC) with 5 mol% catalyst LiPF ₆

In an inerted GC-septum glass with magnetic stirrer core, 1.50 g LiBOB and 0.23 g ground lithium fluoride were dissolved or suspended in 6.8 g PC and 0.59 g of a 10% LiPF ₆ solution in PC was added. To the stirred suspension were 1, 10 g of boron trifluoride etherate injected and then heated to 70 ° C. Samples were taken at certain time intervals and tested for reaction progress by ¹¹ B-NMR:

* indicates the chemical shift of the respective product in the ¹¹ B-NMR spectrum

Example 5: Preparation of LiDFOB from LiBOB, lithium fluoride and BF ₃ in

Tetrahydropyran (THP) without catalyst

In an inerted GC-septum glass with magnetic stirrer core, 1.50 g LiBOB and 0.25 g ground lithium fluoride were dissolved or suspended in 8.5 g THP. 1.10 g of boron trifluoride etherate were injected into the stirred suspension and then heated to 70.degree. Samples were taken at certain time intervals and tested for reaction progress by ¹¹ B-NMR:

* indicates the chemical shift of the respective product in ¹¹ B-NMR

spectrum

Example 6: Preparation of LiDFMB from lithium ö / s (malonato) borate (LiBMB),

Lithium fluoride and BF ₃ in propylene carbonate (PC) without catalyst

In an inertized GC-septum glass with magnetic stirrer core, 1.78 g of LiBMB and 0.21 g of lithium fluoride were suspended in 11 g of PC. To the stirred suspension were 1, 14 g of boron trifluoride etherate injected and then stirred at 100 ° C. Samples were taken at certain time intervals and tested for reaction progress by ¹¹ B-NMR:

Example 7 Preparation of LiDFMB from Lithium O / s (Malonato) Borate (LiBMB),

Lithium fluoride and BF3 in dimethylsulfoxide (DMSO) without catalyst In an inerted GC septum glass with magnetic stirrer, 1.78 g of LiBMB and 0.21 g of lithium fluoride were dissolved or suspended in 10.5 g of DMSO. To the stirred suspension, 1.14 g of boron trifluoride etherate were injected and then stirred at 100 ° C. After a short time, an almost clear reaction solution was formed. Samples were taken at certain time intervals and tested for reaction progress by ¹¹ B-NMR:

NMR spectrum

Claims

claims

1 . Process for the preparation of metal difluoroborates of the general formula wherein M ^{+ is} a monovalent cation selected from the group lithium, sodium, potassium or ammonium NR ₄ ⁺ , wherein R = H, alkyl (C 1 to C 8) and

L is a chelating agent with two terminal oxygen atoms with the general formula

C ² and C ³ are members of a 5- or 6-membered aromatic or heteroaromatic ring (with N, O or S as a heteroelement), the optionally substituted with alkyl, alkoxy, carboxy or nitrile, wherein R ¹ , R ² , Y ³ and Y ⁴ omitted, m = 0 or in the case of 1 mean Y ¹ and Y ² together with C ^{1 is} a carbonyl group and p 0 or 1, by reacting a metal bis (chelato) borate of the formula M [BI_2] with boron trifluoride and a metal fluoride (MF) and / or a metal salt of the chelating ligand (M ₂ L) in an organic aprotic solvent.

2. The method according to claim 1, characterized in that M ⁺ = Li ⁺ and L = C ₂ O ^{2 "} (oxalate) or C ₃ H ₂ O ^2" (malonate) and that as products Lithiumdifluorooxalatoborat (LiDFOB) or Lithiumdifluoromalonatoborat ( LiDFMB).

3. The method according to claim 1 or 2, characterized in that the solvents used are ethers, esters, nitriles, lactones, alkyl carbonates, either in pure form or in any desired mixture.

4. The method according to claim 1 to 3, characterized in that as the solvent preferably carbonic acid esters (dimethyl carbonate, diethyl carbonate, ethylmethyl carbonate, propylene carbonate, ethylene carbonate), cyclic ethers such as tetrahydropyran or tetrahydrofuran, polyethers such as 1, 2-dimethoxyethane or diethylene glycol dimethyl ether, further nitriles such as acetonitrile , Adiponitrile, malononitrile, glutaronitrile and lactones such as v-butyrolactone.

5. The method according to claim 1 to 4, characterized in that the reaction at temperatures of 0 to 250 ° C, preferably from 20 to 150 ° C and preferably from 30 to 130 ° C is performed.

6. The method according to claim 1 to 5, characterized in that the sparingly soluble starting materials, ie the metal fluorides and / or metal chelate salts, in pulverized form, preferably ground, are used.

7. The method according to claim 1 to 6, characterized in that the average particle size of the sparingly soluble starting materials <100 μηη and preferably <50 μηη is.

8. The method according to claim 1 to 7, characterized in that the metal salts MF and / or M ₂ L are used in excess.

9. The method according to claim 1 to 8, characterized in that the metal salts MF and / or M ₂ L with 0.1 to 100 wt -.% Excess, preferably be used with 1 to 20% by weight excess.

10. The method according to claim 1 to 9, characterized in that a catalyst is used to accelerate the reaction.

1 1. A method according to claim I to 10, characterized in that the catalyst contains or consists of a Lewis acid or a substance which can release a Lewis acid in the reaction mixture.

12. The method according to claim I to 1 1, characterized in that the catalyst element compounds of the 2nd - 15th group of the Periodic Table, preferably molecular halides, perfluoroalkyls, perfluoroaryls and / or oxo compounds of boron, aluminum and phosphorus, preferably aluminum alkoxides (AI ( OR) ₃ ), boric acid esters (B (OR) ₃ ), phosphorus oxides or phosphorus halides.

13. The method according to claim I to 12, characterized in that LiPF _{6 is} used as the catalyst.

14. The method according to claim 1 to 13, characterized in that the catalyst in amounts of at most 20 mol%, preferably up to 10 mol% and particularly preferably up to 5 mol%, based on the boron trifluoride used.

15. Use of the products prepared by the process according to the invention as electrolytes or additives in galvanic cells, preferably lithium batteries.